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Chapter 17: Q5P (page 775)

White phosphorous, p4, is produced by the reduction of phosphate rock, Ca3(PO4)2.If exposed to oxygen, the waxy, white solid smokes, bursts into flames, and releases a large quantity of heat. Does the reactionP4(g)+5O2(g)饾啅P4O10(S) have a large or small equilibrium constant? Explain.

Short Answer

Expert verified

The answer is,

Yes, a small equilibrium constant

Step by step solution

01

Equilibrium

The equilibrium state of a reaction is represented using the double-headed arrows and the equilibrium constant is used to denote the scene mathematically. It is the ratio of the concentration of products to the ratio of the concentration of the reactants.

02

Explanation

The equilibrium constant K of a reaction is written as the ratio of the concentration of the products to the concentration of the reactants of the aqueous or gaseous substances. The solid and liquid substances are omitted from the equilibrium constant equation.

Hence the equilibrium constant of the given equation can be written as shown below.

K=1P4O25

Therefore the value of K will be very small.

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Most popular questions from this chapter

What is implied by the word 鈥渃onstant鈥� in the term equilibrium constant? Give two reaction parameters that can be changed without changing the value of an equilibrium constant.

In the 1980s, CFC-11 was one of the most heavily produced chlorofluorocarbons. The last step in its formation is

CCI4(g)+HF(g)鈻�CFCI3(g)+HCI(g)

If you start the reaction with equal concentrations of CCI4and HF, you obtain

equal concentrations of CFCI3and HCl at equilibrium. Are the final

concentrations of CFCI3and HCl equal if you start with unequal

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Question:For the following equilibrium system, which of the changes will form more CaCO3?

CO2(g)+Ca(OH)2(s)鈫�CaCO3(s)+H2O(l)鈭�Ho=-113kJ

(a) Decrease temperature at constant pressure (no phase change)

(b) Increase volume at constant temperature

(c) Increase partial pressure of CO2

(d) Remove one-half of the initial CaCO3

Consider the following reaction:

3Fe(s)+4H2O(g)鈬�Fe3O4(s)+4H2(g)

(a) What is the apparent oxidation state ofFe in Fe3O4 ?

(b) Actually, Fe has two oxidation states in Fe3O4. What are they?

(c) At 900掳C,Kcfor the reaction is 5.1. If 0.050molofH2O(g) and 0.100mol ofFe(s) are placed in a1.0鈭�L container at900掳C , how many grams of Fe3O4 are present at equilibrium?

Note: The synthesis of ammonia is a major process throughout the industrialized world. Problems 17.99 to 17.105 refer to various aspects of this all-important reaction:

N2(g)+3H2(g)鈬�2NH3(g)鈥夆赌夆赌�螖贬rxn掳=鈭�91.8kJ

The formation of methanol is important to the processing of new fuels. At 298K,KP=2.25脳104for the reaction


localid="1662026070224" CO(g)+2H2(g)鈬�CH3OH(I)

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